Both Nitrogen and Hydrogen exist as diatomic molecules. Take a look at the oxidation numbers of the elements and refer to common ions and compounds. Knowing this, you should be able to complete the reactions and balance them on your own.

t!m-- Yes, I know a little about those, I just took notes on them. ^_^

The first one is a little long...what would I have to do with that one?

Second -- Decomposition?
Third -- Synthesis?
Fourth -- Single Replacement?

Was what I had down wrong? This is what threw me, "The products must conform to the rules you learned in assignments 3.05 and 3.06. In other words, the new products you write down must be neutral, that is the positive and negative charges must cancel out. For instance, if Lithium oxide is a new product, Lithium has a charge of +1, Oxygen a charge of –2. So the new compound formed would be: Li2O" I had trouble with this last year and since learning it on my own wasn't working, I got a tutor. However, my tutor began to touch on this but then I had to leave and that was the last session I had so I was left sort of hanging there.:rofl: I'll have to try and find something about this in the text book I was loaned...

Alright, let me see if I got this...to do this, I have to look at the electrons and protons involved, right?

H2 + O2

Hydrogen has one electron and one proton. In order for it to have a noble gas configuration, it would be easier for it to lose it's one electron than it would be to gain seven more...so, after it loses it, it would be positive (+1). Oxygen has eight electrons and eight protons...it has six valence electrons. It would be easier for it to gain two electrons than it would be to lose six so it would become negative (-2).